/ Preparation Chemistry Acids, Bases and Salts
Sodium chlorate (NaClO3) is a crystalline, pale yellow to white coloured inorganic salt of sodium and chloric acid. It is perfectly soluble in water and is hygroscopic in nature. They are available in powdered, spray or pellet forms.
It is a strong oxidising agent, therefore contact with organic compounds or any easily oxidised materials will lead to explosions. Excessive heat above 300⁰C will decompose sodium chlorate to sodium chloride releasing oxygen, further increasing the intensity of fire. Hence commercial formulations are normally mixed with fire retardants like sodium metaborate to prevent accidental explosions.
Sodium Chloride is also toxic to both plants and animals. A dose with few grams of chlorate is found to be lethal for human beings.
- Laboratory Preparation
- Industrial Preparation
- Uses of Sodium Chlorate
- Sodium Chlorate in class 10
- Sodium Chlorate in Class 11
- Sodium Chlorate in Class 12
- FAQs on Sodium Chlorate
Laboratory Preparation
Chlorine (Cl2) is added to hot and concentrated Sodium Hydroxide (NaOH).
6NaOH + 3Cl2 → 5NaCl + NaClO3 + 3H2O
This is an example of a disproportionation reaction, where the oxidation state of chlorine is both reduced to -1 (in NaCl) and oxidized to +5 (in NaClO3) from its initial 0 oxidation state.
Industrial Preparation
Sodium chlorate is industrially prepared by the electrolysis of hot aqueous sodium chloride solution (brine).
NaCl + 3H2O → NaClO3 + 3H2
It is important to maintain the pH and temperature (about 50 -70 ⁰C), else the product formed will be different.
Uses of Sodium Chlorate
Sodium Chlorate is mainly used to manufacture chlorine dioxide (ClO2), a bleaching agent in the paper industry to bleach pulp to produce pure white papers.
Earlier, it was commonly used as a non-selective herbicide to control growth of certain plants and weeds. After identifying its possible health risks, its usage has been considerably reduced and is even banned in some places.
As sodium chlorate decomposes at high temperature and releases oxygen, it is used in chemical oxygen generators, such as the one in aircrafts to provide emergency oxygen to passengers. The pulling of the emergency mask triggers the process of decomposition. The initial heat required is produced by mixing sodium chlorate and a bit of iron powder. The trace amounts of chlorine released is absorbed by barium peroxide.
2NaClO3 → 2NaCl + 3 O2
In the Solidox welding system, sodium chlorate pellets mixed with combustible fibres are used to produce oxygen.
At times, sodium chlorate mixed with sucrose sugar is used as a highly explosive fuel in airtight spaces. This process is also known as oxygenless combustion, as the reaction takes place under limited oxygen supply and the oxygen required is produced as the reaction progresses.
Sodium Chlorate in class 10
In Chapter 2, Acids, Bases and Salts, the formation of salts is explained.
Sodium Chlorate in Class 11
In Chapter 10, The s-Block Elements – A few compounds of sodium is introduced and formation similar metal compounds are explained. In Chapter 14, Environmental Chemistry, Sodium Chlorate is classified as a toxic soil pollutant.
Sodium Chlorate in Class 12
In Chapter 7, The p-Block Elements – Chlorine and its compounds are introduced.
FAQs on Sodium Chlorate
Q: What is hygroscopy?
Q: What is a disproportionation reaction?
Q: What is meant by fire retardants?
Q: What is an Oxidising agent?
Q: What is Electrolysis?
Chemistry Acids, Bases and Salts Exam
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